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Chemistry
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11 Dec 2019

The decomposition of SO2Cl2 is first order in SO2Cl2 and has a rate constant of 1.36×10−4 s−1 at a certain temperature.
Find the half life?
How long will it take for the concentration of SO2Cl2 to decrease to 25% of its initial concentration?
If the initial concentration of SO2Cl2 is 1.00 M, how long will it take for the concentration to decrease to 0.80 M ?
If the initial concentration of SO2Cl2 is 0.125 M , what is the concentration of SO2Cl2 after 210 s ?
If the initial concentration of SO2Cl2 is 0.125 M , what is the concentration of SO2Cl2 after 470 s ?

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Nestor Rutherford
Nestor RutherfordLv2
13 Dec 2019

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Related questions

The decomposition reaction SO2Cl2(g) → SO2(g) + Cl2(g) is first order, with a rate constant of 2.2 × 10–5 s –1 at 320°C. The partial pressure of SO2Cl2(g) in a sealed vessel at 320°C is initially 1.0 atm. How long will it take for the partial pressure of SO2Cl2(g) to fall to 0.50 atm?

As described in Exercise 14.41, the decomposition of sulfuryl chloride (SO2Cl2) is a first-order process. The rate constant for the decomposition at 660 K is 4.5×10-2 s–1. (a) If we begin with an initial SO2Cl2 pressure of 450 torr, what is the partial pressure of this substance after 60 s? (b) At what time will the partial pressure of SO2Cl2 decline to one-tenth its initial value?

The decomposition of sulfuryl chloride (SO2Cl2) is a first-order process. The rate constant for the decomposition at 660 K is 4.5×10−2s−1. If we begin with an initial SO2Cl2 pressure of 500 torr , what is the partial pressure of this substance after 70 s ?

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